What is the Gibbs energy of the following reaction?
`Zn(s)+Cu^(2+) (aq) rarr Zn^(2+)(aq)+Cu^(2+) (s), E_("cell")^(@)=1.1 V`

For the cell reaction Zn(s) + Cu^(2+)(aq) rarr Cu(s) + Zn^(2+)(aq) E_("cell")^(@) = 1.10 V, DeltaG^(@) is :

The cell in which the following reaction occur. 2Zn(s)+2Cu^(2+)(aq) rarr 2Zn^(2+)(aq)+2Cu(s)E_(cell)^@=1.10 volt at 298K. Calculate the standard Gibbs energy and the equilibrium constant.

Derive Nerst equation for EMF of the following cell. Zn (s) + Cu^2+ (aq) rarr Zn^2+ (aq) + Cu(s)

Represent the galvanic cell in which the reaction Is: Zn(s)+Cu^(2+) (aq) rarr Zn^(2+) (aq)+Cu(s)

Write Nernst equation for the following cell reaction : Zn(s) | Zn^(2+)(aq)|| Cu^(2+)(aq) | Cu(s)

Calculate the equilibrium costant log (K_(c)) for the reaction Zn(s)+Cu^(2+)(aq)rarrZn^(2+)(aq)+Cu(s) [Given E_(cell)^(2)=1.1 V ]

Calculate the standard free energy change for the following reaction Zn(s) + Cu^(2+)(aq) to Zn^(2+) (aq) + Cu(s) Given : Delta_fG^@ [Cu^(2+)(aq)] = 65.0kJ mol^(-1) Delta_f G^@ [ Zn^(2+) (aq)] = -147.2 kJ mol^(-1)

E^(@) for the electrochemical cell Zn(s) | Zn^(2+)1M (aq)|| Cu^(2+) 1M(aq)| Cu (s) is 1.10 V at 25^(@) C. The equilibrium constant for the cell reaction, Zn(s)+Cu^(2+) (aq.) rarr Zn^(2+) (aq.) + Cu(s) will be:

The standard electrode potential for Daniell cell is 1. IV. Calculate the standard Gibbs energy for the reaction: Zn(s) + Cu^(2+) (aq) rarr Zn^(2+)(aq) + Cu(s)